50 mL of 0.20M HCl is tirated with 0.25M NaOH a. What is the initial pH of the a
ID: 681459 • Letter: 5
Question
50 mL of 0.20M HCl is tirated with 0.25M NaOH a. What is the initial pH of the acid solutions? b. What is the pH after the addition of 20.0 mL of NaOH? c. What is the pH at the equivalence point? e. What is the pH after the addition of 45.0 mL? Show ALL work for full points. 50 mL of 0.20M HCl is tirated with 0.25M NaOH a. What is the initial pH of the acid solutions? b. What is the pH after the addition of 20.0 mL of NaOH? c. What is the pH at the equivalence point? e. What is the pH after the addition of 45.0 mL? Show ALL work for full points.Explanation / Answer
HCl + NaOH -----------> NaCl +H2O a) pH = - log [ H+] = - log ( 0.2) = 0.7 b) HCl + NaOH -----------> NaCl + H2O Before rxn 0.05 L *0.2 M 0.02 L * 0.25 M = 0.01 0.005 moles Afterrxn 0.005 moles 0 0.005 moles [H+ ] = 0.005 moles / 0.07 L = 0.071 pH = 1.14 c) At equivalence point pH 7. d) HCl + NaOH -----------> NaCl + H2O Before rxn 0.05 L *0.2 M 0.045 L * 0.25 M = 0. 01 0.01125 moles Afterrxn 0 0.00125 0.1 [OH-] = 0.00125 moles / 0.095 L =0.0131 M pOH = 1.88 pH = 12.12 Before rxn 0.05 L *0.2 M 0.045 L * 0.25 M = 0. 01 0.01125 moles Afterrxn 0 0.00125 0.1 [OH-] = 0.00125 moles / 0.095 L =0.0131 M pOH = 1.88 pH = 12.12Related Questions
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